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Complete the following in lab, obtain a staff signature, and submit. 1) Fill in the table with your observations. 2) Write the balanced half-reaction equations and the balanced overall equation for the Zn−Mg cell. 3) Give three reasons, with explanations, for the difference between E∘ calculatod and Emeasured. . ​. 4) Fill in the table with your observations.
3) Give three reasons, with explanations, for the difference between E∘ calculated and E moasured. 4) Fill in the table with your observations. 5) Write the balanced equation for the chemistry that occurs when NH3(00)​ is added to one of the half-cells. 6) Explain the change in voltage going from the initial cell to the one containing NH3​(a). Consider thermodynamics and equilibrium in your response. Uniets otherwise ypeellat, this werk by Wothingens State Cotleges is leensed under a 7
7) Complete the table with your observations. 8) Attach your signed, photocopied lab notebook pages.
A Concentration Cell A special type of a non-standard cell is a concentration cell. You will irvestigate the behavior of Cu-Cu concentration cell. A standard Cu-Cu cell potential would be zero. Diluting one of the half-cells creates a measurable potential difference. Changes to the concentration can also be made by complexing or precipitating the metal lons. You will observe how these concentration changes affect the voltage. By entering E and E e and the known concentration of one half-cell into the Nemst equation the unknown concentration of a test solution in the other half-cell can be calculated. This is the basis for determining pH using a pH meter and fincing Ksp ​ for nearly insoluble substances. An Electrolytic Cell Your final investigation will involve the construction of an electrolytic cell. An electrolytic cell is a non-spontaneous cell that must have energy continuously inputted to force electrons from anode to cathode. Electrolysis is the method used to reduce ionic metals and oxidize ionic non-metals to pure elements. Electroplating a metal on another metal or plastic is one application of this method. To convert the galvanic Cr-Ni cell into an electrolytic cell, the voltmeter is replaced by a power source that inputs more than 0.50 V to move electrons from the Ni to the Cr. This reversed flow makes Ni the anode (+) and Cr the cathode (-). Symbolically, changing a galvanic cell to an electrolytic cell simply swaps the names anode and cathode and reverses the flow of electrons. 3 Unless otherwise specified, this wort by Washington Sute Colinged allicensed unter?
You will be constructing a Cu−Cu electrolytic cell which reduces Cu2+ to Cu for purpose of measuring Avogadro's number (NA​). After a period of reduction the mass by the Cu cathode will be measured and with this the moles of electrons used will be determined. mole−=massCu ×63.546 g1molCu​×molCu2 mole−​ The total charge transferred will be calculated from the current (amperes = Coulombs/sec that flows for a measured time period (seconds) during the reduction. Given that the chat on 1 electron is 1.60×10−19 Coulombs, the total number of electrons transferred is: Ne​== current × time ×e−per charge  Ne−​=1.602×10−19C/e−sC​×s​ Avogadro's number is easily calculated from the quantity molel −Ne−​​=NA​ Procedure Work in groups of 2 , sign out the following equipment: a Fluke multimeter, a set of 20 mL beakers, a transformer, a U-tube, a LabQuest to use as a timer, and the necessary electric leads with attached alligator clips and/or jacks. Galvanic Cells 1. Start the construction of the four different half-cells by filling each 20 mL beaker 3/4 ful with the appropriate 0.1M aqueous solution; Cu(NO3​)2​,ZnNO3​,MgSO4​, and FeSO4​ (ma fresh). Complete the construction by: (1) sanding strips of copper, zinc, magnesium, anc iron, (2) washing each strip with deionized water and then drying, and (3) folding the eac strip over the lip of its respective beaker making sure the strip is partially immersed in the solution. These strips are the half-cell electrodes. 2. Prepare the 0.100MFeSO4​ solution by dissolving 0.556. grams of FeSO4​⋅7H2​O in 20.00 mL of Di water. 3. To prepare the Cu-Zn cell, clip a lead to each half-cell electrode. Attach the jack of the black lead to the COM (common) port (black) and the red lead jack to the V port (red). Th is the external circuit. Place a strip of filter paper on a watch-glass and thoroughly moiste Urieis otherwse specifid, ths work by Washisgton 92 ste Coleses is licenaed unser a